Question 1

At 570. mm Hg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C?

Accepted Answer

A)  1560 mmHg 
B)  210. mmHg 
C)  700. mmHg 
D)  690. mmHg 
E)  470. mmHg 
A)  1560 mmHg 
B)  210. mmHg 
C)  700. mmHg 
D)  690. mmHg 
E)  470. mmHg

Question 2

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr?

Accepted Answer

A)  530 mL 
B)  450 mL 
C)  970 mL 
D)  240 mL 
E)  400 mL 
A)  530 mL 
B)  450 mL 
C)  970 mL 
D)  240 mL 
E)  400 mL

Question 3

Match the correct formula with the gas law name given.
-Ideal Gas Law

Accepted Answer

A) $\frac { P _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } } { T _ { 2 } }$ 
B) $\frac { V _ { 1 } } { n _ { 1 } }$ = $\frac { V _ { 2 } } { n _ { 2 } }$ 
C) $\frac { V _ { 1 } } { T _ { 1 } }$ = $\frac { V _ { 2 } } { T _ { 2 } }$ 
D) PV = nRT 
E) $\frac { P _ { 1 } V _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } V _ { 2 } } { T _ { 2 } }$
F)P1V1 = P2V2
G)mass/volume
H)PT = P1 + P2 + P3 ... 
A) $\frac { P _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } } { T _ { 2 } }$ 
B) $\frac { V _ { 1 } } { n _ { 1 } }$ = $\frac { V _ { 2 } } { n _ { 2 } }$ 
C) $\frac { V _ { 1 } } { T _ { 1 } }$ = $\frac { V _ { 2 } } { T _ { 2 } }$ 
D) PV = nRT 
E) $\frac { P _ { 1 } V _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } V _ { 2 } } { T _ { 2 } }$
F)P1V1 = P2V2
G)mass/volume
H)PT = P1 + P2 + P3 ...

Question 4

A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. How many gas particles are in this bubble?

Accepted Answer

A)  1.5 × 1022 gas particles 
B)  0.25 gas particles 
C)  6.02 × 1023 gas particles 
D)  490 gas particles 
E)  2.9 × 1026 gas particles 
A)  1.5 × 1022 gas particles 
B)  0.25 gas particles 
C)  6.02 × 1023 gas particles 
D)  490 gas particles 
E)  2.9 × 1026 gas particles

Question 5

What unit of temperature is used in gas law calculations?

Accepted Answer

A)  degrees Fahrenheit 
B)  degrees Celsius 
C)  Kelvin 
D)  either degrees Celsius or degrees Fahrenheit 
E)  either degrees Celsius or Kelvin 
A)  degrees Fahrenheit 
B)  degrees Celsius 
C)  Kelvin 
D)  either degrees Celsius or degrees Fahrenheit 
E)  either degrees Celsius or Kelvin

Question 6

The mathematical expression of the ideal gas law is

Accepted Answer

A)  P1V1 = P2V2 
B)  $\frac { P _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } } { T _ { 2 } }$ 
C)  $\frac { P _ { 1 } } { V _ { 1 } }$ = $\frac { P _ { 2 } } { V _ { 2 } }$ 
D)  PV = nRT 
E)  PT = P1 + P2 + P3 
A)  P1V1 = P2V2 
B)  $\frac { P _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } } { T _ { 2 } }$ 
C)  $\frac { P _ { 1 } } { V _ { 1 } }$ = $\frac { P _ { 2 } } { V _ { 2 } }$ 
D)  PV = nRT 
E)  PT = P1 + P2 + P3

Question 7

A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 330 mmHg and the partial pressure of the oxygen is 1.0 atm, what is the total pressure of the mixture in torr?

Accepted Answer

A)  330 torr 
B)  430 torr 
C)  760 torr 
D)  1.4 torr 
E)  1100 torr 
A)  330 torr 
B)  430 torr 
C)  760 torr 
D)  1.4 torr 
E)  1100 torr

Question 8

Match the correct formula with the gas law name given.
-Avogadro's Law

Accepted Answer

A) $\frac { P _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } } { T _ { 2 } }$ 
B) $\frac { V _ { 1 } } { n _ { 1 } }$ = $\frac { V _ { 2 } } { n _ { 2 } }$ 
C) $\frac { V _ { 1 } } { T _ { 1 } }$ = $\frac { V _ { 2 } } { T _ { 2 } }$ 
D) PV = nRT 
E) $\frac { P _ { 1 } V _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } V _ { 2 } } { T _ { 2 } }$
F)P1V1 = P2V2
G)mass/volume
H)PT = P1 + P2 + P3 ... 
A) $\frac { P _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } } { T _ { 2 } }$ 
B) $\frac { V _ { 1 } } { n _ { 1 } }$ = $\frac { V _ { 2 } } { n _ { 2 } }$ 
C) $\frac { V _ { 1 } } { T _ { 1 } }$ = $\frac { V _ { 2 } } { T _ { 2 } }$ 
D) PV = nRT 
E) $\frac { P _ { 1 } V _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } V _ { 2 } } { T _ { 2 } }$
F)P1V1 = P2V2
G)mass/volume
H)PT = P1 + P2 + P3 ...

Question 9

According to Boyle's Law, the pressure of a gas increases as the volume decreases because

Accepted Answer

A)  the gas particles get bigger. 
B)  the kinetic energy of the gas particles increases. 
C)  the temperature of the gas increases. 
D)  the gas particles strike the walls of the container with more force. 
E)  the gas particles strike the walls of the container more often. 
A)  the gas particles get bigger. 
B)  the kinetic energy of the gas particles increases. 
C)  the temperature of the gas increases. 
D)  the gas particles strike the walls of the container with more force. 
E)  the gas particles strike the walls of the container more often.

Question 10

Nitrogen makes up about __________ percent of the atmosphere.

Accepted Answer

The answer of Nitrogen makes up about __________ percent of...

Question 11

At STP, how many moles of helium would occupy 1.00 L?

Accepted Answer

A)  2.24 moles 
B)  224 moles 
C)  22.4 moles 
D)  0.446 moles 
E)  0.0446 moles 
A)  2.24 moles 
B)  224 moles 
C)  22.4 moles 
D)  0.446 moles 
E)  0.0446 moles

Question 12

When the combined gas law is rearranged to solve for V2, the following is the correct expression: V2=

Accepted Answer

A)  T2 T1 V1/P2P1 
B)  P1V1T2/P2T1 
C)  P1V1T1/P2T2 
D)  P2T2/P2V1T1 
E)  P1V1/T1 - P2/T2 
A)  T2 T1 V1/P2P1 
B)  P1V1T2/P2T1 
C)  P1V1T1/P2T2 
D)  P2T2/P2V1T1 
E)  P1V1/T1 - P2/T2

Question 13

1 mole of a gas occupies 22.4 L at

Accepted Answer

A)  0 °C and 0.50 atm. 
B)  0 °C and 760 mmHg. 
C)  100 °C and 1 atm. 
D)  100 °C and 10 atm. 
E)  0 K and 1 atm. 
A)  0 °C and 0.50 atm. 
B)  0 °C and 760 mmHg. 
C)  100 °C and 1 atm. 
D)  100 °C and 10 atm. 
E)  0 K and 1 atm.

Question 14

A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What will be the gas pressure when the temperature changes to 450 K?

Accepted Answer

A)  1.5 atm 
B)  0.94 atm 
C)  0.47 atm 
D)  2.1 atm 
E)  1.1 atm 
A)  1.5 atm 
B)  0.94 atm 
C)  0.47 atm 
D)  2.1 atm 
E)  1.1 atm

Question 15

The boiling point of water at sea level is 100 °C. At higher altitudes, the boiling point of water will be

Accepted Answer

A)  lower, because temperatures are lower. 
B)  lower, because the atmospheric pressure is lower. 
C)  higher, because the altitude is greater. 
D)  higher, because there are fewer water molecules in the air. 
E)  the same, because water always boils at 100 °C. 
A)  lower, because temperatures are lower. 
B)  lower, because the atmospheric pressure is lower. 
C)  higher, because the altitude is greater. 
D)  higher, because there are fewer water molecules in the air. 
E)  the same, because water always boils at 100 °C.

Question 16

Indicate the effect on the pressure of the following change.
-Some molecules of gas are removed (V, T constant).

Accepted Answer

A) increases 
B) decreases 
C) no change 
A) increases 
B) decreases 
C) no change

Question 17

1 mmHg is the same as 760 atm.

Accepted Answer

A) True 
 B)False

Question 18

Which measurement describes the pressure of a gas?

Accepted Answer

A)  315 K 
B)  1.2 g/L 
C)  2.5 L 
D)  725 mmHg 
E)  0.45 moles 
A)  315 K 
B)  1.2 g/L 
C)  2.5 L 
D)  725 mmHg 
E)  0.45 moles

Question 19

A tank contains helium gas at 490 mmHg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm?

Accepted Answer

A)  2.1 atm 
B)  0.55 atm 
C)  1.0 × 103 atm 
D)  1.5 atm 
E)  1600 atm 
A)  2.1 atm 
B)  0.55 atm 
C)  1.0 × 103 atm 
D)  1.5 atm 
E)  1600 atm

Question 20

At STP, what is the volume of 4.50 moles of nitrogen gas?

Accepted Answer

A)  167 L 
B)  3420 L 
C)  101 L 
D)  60.7 L 
E)  1230 L 
A)  167 L 
B)  3420 L 
C)  101 L 
D)  60.7 L 
E)  1230 L

Exam 7: Gases

At 570. mm Hg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C?

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr?

Match the correct formula with the gas law name given. -Ideal Gas Law

A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. How many gas particles are in this bubble?

What unit of temperature is used in gas law calculations?

The mathematical expression of the ideal gas law is

A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 330 mmHg and the partial pressure of the oxygen is 1.0 atm, what is the total pressure of the mixture in torr?

Match the correct formula with the gas law name given. -Avogadro's Law

According to Boyle's Law, the pressure of a gas increases as the volume decreases because

Nitrogen makes up about __________ percent of the atmosphere.

At STP, how many moles of helium would occupy 1.00 L?

When the combined gas law is rearranged to solve for V2, the following is the correct expression: V2=

1 mole of a gas occupies 22.4 L at

A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What will be the gas pressure when the temperature changes to 450 K?

The boiling point of water at sea level is 100 °C. At higher altitudes, the boiling point of water will be

Indicate the effect on the pressure of the following change. -Some molecules of gas are removed (V, T constant).

1 mmHg is the same as 760 atm.

Which measurement describes the pressure of a gas?

A tank contains helium gas at 490 mmHg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm?

At STP, what is the volume of 4.50 moles of nitrogen gas?

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When the combined gas law is rearranged to solve for V₂, the following is the correct expression: V₂=